Process for preparing finely divided highly reactive magnesium and use thereof

ABSTRACT

The present invention relates to a process for preparing a finely divided, highly reactive magnesium from magnesium hydride, magnesium anthracene and/or its derivatives or magnesium butadiene and/or its alkyl or phenyl derivatives, which process is characterized in that the respective magnesium-containing compound is thermally decomposed at a pressure from 10 -6  to 1 bar, the decomposition being carried out in the presence of a co-reactant of a consecutive reaction, or such co-reactant being added only after completion of the precipitation of the magnesium, or in the absence of such co-reactant, the magnesium obtained by said decomposition being isolated as a powder, and to the use of the finely divided, highly reactive magnesium for inserting magnesium into poorly reactive C-X bonds, wherein X denotes heteroatoms such as halogen, oxygen, sulfur, nitrogen, phosphorus, and the resulting organomagnesium compound may be used in a consecutive reaction according to a per se known method, and for the reversible preparation of active magnesium hydride by reaction with molecular hydrogen at a pressure of from 1 to 2 bar and at a temperature of from 150° C. to 250° C.

The invention relates to a process for preparing a finely divided,highly reactive magnesium and the use thereof.

Activated forms of metallic magnesium are used to an increasing extentin chemical syntheses, more specifically for Grignard reactions, asreducing agents, for dehalogenation reactions and the like. Thereby,most of said reactions can be effected with a substantially higherefficiency than, e.g., by using commercially available magnesium powder,while other reactions have only become realizable therewith (cf., e.g.,Y.-H. Lai, Synthesis 585 (1981); W. Oppolzer in "Current Trends inOrganic Synthesis", Ed. H. Nozaki, Pergamon Press 1983, p. 131).According to R. D. Rieke, magnesium can be obtained in an active form byreduction of magnesium halides with alkali metals, more particularlywith potassium, in tetrahydrofuran (THF) (Acc. Chem. Res. 10, 301(1977)) or 1,2-dimethoxyethane, optionally with the addition ofnaphthalene as an electron transfer agent (Arnold & Kulenovic, Synth.Commun. 7, 223 (1977); Rieke et al., J. Org. Chem. 46 4323 (1981). Thesemethods have disadvantages inasmuch as that activated magnesium isobtained suspended in THF or 1,2-dimethoxyethane as a mixture with therespective alkali metal halide and mostly also with the alkali metal sothat for the preparation of active magnesium by said route equimolaramounts of alkali metal, e.g. metallic potassium, are required.

It is the object of the present invention to provide a process for thepreparation of highly active magnesium, which process is free from theaforementioned drawbacks and, in addition, is suitable for being carriedout on a larger scale.

There has been known that an equilibrium exists between metallicmagnesium and hydrogen, on the one hand, and magnesium hydride, on theother hand, which equilibrium inherently is temperature-dependent andreversible:

    Mg+H.sub.2 ⃡MgH.sub.2, ΔH=-74,8 kJ/mol   (1)

At room temperature and under regular pressure, the equilibrium ofequation (1) is almost completely on the magnesium hydride side. Withincreasing temperature, the hydrogen partial pressure of magnesiumhydride increases and, for example, reaches the values of 1, 2 and 5.5bar at a temperature of 284° C., 310° C. and 350° C., respectively.However, the hydrogenation of commercially available magnesium in theabsence of catalysts well as the thermal decomposition of the formedmagnesium hydride proceed at an extremely low speed even at atemperature of about 400° C. (cf., e.g., Stander, Z. fur physikal. Chem.Neue Folge 104, 229 (1977)). In addition, in the thermal decompositionof the magnesium hydride prepared at a high temperature there is formeda magnesium metal having a low chemical reactivity, so that said routewill hardly be suitable as a method for activating magnesium.

According to the European Patent Specification No. 0 003 564 (toApplicants) a process has become known which allows magnesium to behydrogenated to give magnesium hydride under mild conditions (e.g. atfrom 20° C. to 60° C. and from 1 to 80 bar) by means of the homogeneouscatalysts as described therein.

Now, surprisingly there has been found that a finely divided, highlyreactive magnesium suspended in a solvent or, upon respective work-up, apyrophoric magnesium powder having an unexpectedly high chemicalreactivity is formed, when said magnesium hydride generated in thepresence of a homogeneous catalyst is thermally dehydrogenated.Therefore, a method according to the invention for preparing a highlyreactive and very finely divided magnesium comprises the thermaldehydrogenation under reduced pressure of magnesium hydride having beenprepared according to a per se known process.

According to the U.S. Patent Specifications No. 3,351,646, 3,354,190 and3,388,179 metallic magnesium in THF will undergo an addition reaction toanthracene and other condensed aromatic ring systems and to butadieneand other conjugated dienes to form the corresponding magnesium adductsof said hydrocarbons, magnesium anthracene, magnesium butadiene etc. Inaccordance with our findings, the adducts magnesium anthracene.3 THF,magnesium butadiene.2 THF etc. are in a temperature-dependent,reversible equilibrium with their respective organic constituents andmagnesium metal (Eqns. 2 and 3, respectively), a low temperaturefavoring the adduct formation.

There has now surprisingly been found that a finely divided, highlyreactive magnesium suspended in a solvent or, upon respective work-up, amagnesium powder having an extremely high chemical reactivity is formed,when magnesium anthracene, magnesium butadiene and/or adducts ofmagnesium to other conjugated dienes having the general formula R¹-CH=CR² -CH=CH-R³, wherein R¹, R² and R³ may be same or different andrepresent H, a linear or branched alkyl group having from 1 to 6 carbonatoms or a phenyl residue, are decomposed to form metallic magnesiumupon shifting the equilibria shown by the following equations 2 and 3from the right to the left by raising the temperature and/or reducingthe concentrations of anthracene and THF, or diene and THF,respectively. ##STR1##

Therefore, another method according to the invention for activatingmagnesium comprises first reacting a commercially available magnesium ina per se known manner with anthracene, butadiene or a differentconjugated dienes having the general formula R¹ -CH=CR² -CH=CH-R³,wherein R¹, R² and R³ may be same or different and represent H, a linearor branched alkyl group having from 1 to 6 carbon atoms or a phenylresidue, in THF to form magnesium anthracene.3 THF, magnesiumbutadiene.2 THF etc. (shifting the equilibria according to the equations2 and 3, respectively, from the left side to the right side) andsubsequently producing the activated magnesium by increasing thetemperature and/or reducing the concentrations of anthracene and THF ordiene and THF etc. (shifting back the equilibria according to theequations 2 and 3, respectively, from the right side to the left side)in accordance with the instant process.

In a preferred embodiment of the present invention one procedure foractivating the magnesium comprises hydrogenating commercially availablemagnesium according to the process described in the European PatentSpecification No. 0 003 564 to form magnesium hydride and subsequentlythermally dehydrogenating the magnesium hydride having been thusproduced at a temperature in excess of 300° C. under atmosphericpressure, and preferably in excess of 250° C. under reduced pressure.The hydrogen obtained thereby may be conveniently recycled and used forhydrogenating another magnesium batch in accordance with thehomogeneously catalytic process according to the No. EP-A-0 003 564,whereby an economic process for preparing activating magnesium fromcommercially available magnesium has been provided.

In a further preferred embodiment of the present invention acommercially available magnesium is reacted in a per se known step withanthracene or one of its alkyl or phenyl derivatives according toequation (2), or with a conjugated diene having the general formula R¹-CH=CR² -CH=CH-R³, wherein R¹, R² and R³ may be same or different andrepresent H, a linear or branched alkyl group having from 1 to 6 carbonatoms or a phenyl residue according to equation (3), and the resultingorganomagnesium compound is thermolyzed at an elevated temperature invacuo or at atmospheric pressure.

The preferred range of temperatures for the decomposition of magnesiumanthracene.3 THF or of magnesium adducts to substituted anthracenes inthe solid state is between +70° C. and +170° C. In an inert organicsolvent the decomposition is effected under atmospheric pressure at atemperature of from +20° C. to +100° C. As the inert organic solventsthere may be used aliphatic, cycloaliphatic and aromatic hydrocarbons aswell as open-chain aliphatic ethers such as diethyl ether and dibutylether.

The preferred reaction temperature for the decomposition of magnesiumbutadiene.2 THF and of magnesium adducts to optionally substitutedconjugated dienes, e.g. 1,4-diphenylbutadiene or isoprene, are from +20°C. to +150° C. As a solvent there is used one of the above-mentionedinert organic solvents.

In the place of magnesium anthracene or magnesium butadiene,respectively, there may also be employed the magnesium adducts to thealkyl or phenyl derivatives thereof, e.g. 1,4-diphenyl butadiene orisoprene, for the preparation of finely divided, reactive magnesium,while in the place of THF as a solvent there may be used2-methyltetrahydrofurane or THF in combination withN,N,N',N'tetramethylethylenediamine (TMEDA) or 1,2-dimethoxyethane.

The decomposition of said thermolabile organomagnesium compounds mayoptionally be accelerated by means of a catalyst or promoter which, inaddition, possibly may positively affect the properties of the activemagnesium (particle size, particle shape, (specific) surface area, typeand amount of adsorbed materials); organic halogen compounds, e.g.ethylbromide, 1,2-dichloroethane and 1,2-dibromoethane, and magnesiumhalides may be used as such compounds.

The decomposition of the thermolabile organomagnesium compounds to formhighly reactive magnesium optionally may also be accelerated by somephysical technique (ultrasonic treatment, light irradiation, mechanicaleffects).

The formation of active magnesium may be effected in the presence of thematerials which are to react with the active magnesium (such as, e.g.,organic halogen or phosphorus compounds) or to interact with the activemagnesium (such as, e.g., inorganic carriers at the surface of which theactive magnesium is to be adsorbed). In these cases the active magnesiummay be produced at a temperature substantially lower than +20° C., e.g.at -70° C. or even less, as it is continuously removed from theequilibrium state (equations 2 or 3, respectively) by the directreaction with the reactants, e.g. the organic halogen or phosphoruscompounds.

On the other hand, the materials with which the highly active magnesiumpowder prepared according to the invention is intended to react may alsobe added to the system after the deposition of the active magnesium hasbeen completed. Upon completion of one cycle of the preparation of theactive magnesium, the recovered organic components anthracene,butadiene, THF etc. may be employed to activate another magnesium batch,which process may optionally be operated in a circulation system.

The active magnesium obtainable by the process according to theinvention is distinguished by having a particularly high (specific)surface area; thus, e.g., the specific surface area of the magnesium asproduced by the thermal decomposition of magnesium anthracene.3 THFunder vacuum is 62 m² /g.

The high chemical reactivity, as compared to that of commerciallyavailable magnesium powder, of the magnesium obtainable by the presentprocess, is evident from, inter alia, that it can be inserted in poorlyreactive C-X bonds wherein X denotes hetero atoms such as halogen,oxygen, sulfur, nitrogen, phosphorus and the like.

Thus, the active magnesium obtained by the thermolysis of the magnesiumhydride prepared in the homogeneous catalytic reaction does alreadyreact in THF under mild conditions with aryl chlorides, which arebelieved to be particularly non-reactive in the Grignard reaction, toform the corresponding Grignard compounds in high yields. Allylchlorides can be converted into the Grignard compounds by means of theactive magnesium obtained by the process according to the invention at atemperature as low as -50° C., whereby the Wurtz dimerization of theorganic radicals which at higher temperatures increasingly interfereswith the conventional Grignard reactions can be almost completelysuppressed. For the preparation of the allyl Grignard compounds, thereis preferably employed the variant of the process according to thepresent invention wherein the highly reactive magnesium is produced at alow temperature in the presence of the respective allyl halide.

There has further been known from the literature (and confirmed by owncontrol experiments) that isobutyl chloride does not react nor formorganomagnesium compounds with normal magnesium in hydrocarbons (D. B.Malpass et al. in Kirk-Othmer, Encycl. Chem. Techn., Vol. 16, 3rdedition, p. 555). In the reaction of isobutyl chloride with activemagnesium, obtained by thermolysis of magnesium anthracene in toluene orheptane, respectively, isobutyl magnesiumchloride was obtained in ayield of about 30% (no optimization was attempted in the experiments).

The high reactivity of the active magnesium obtainable by thethermolysis of magnesium hydride prepared in the homogeneous catalyticreaction or of the magnesium anthracene or magnesium diene,respectively, is particularly clearly demonstrated by its cleavagereaction with THF with inserting the metal into a carbon-oxygen bond toform 1-oxa-2-magnesia-cyclohexane. ##STR2##

Conventional types of magnesium are considered to be inert to THF; theformation of the 1-oxa-2-magnesia-cyclohexane by cleavage of THF withmetallic magnesium so far has only been observed when "Rieke magnesium"(Bickelhaupt et al., Heterocycles 7, 237 (1977)) was employed.

The results of several experiments show that1-halogenophospholenium-halides (such as, e.g., 1) can be reduced withactive magnesium obtained according to the invention from magnesiumhydride produced in the homogeneous catalytic reaction to give thecorresponding 3-phospholenes (2) at lower reaction temperatures and withsubstantially higher yields than has been possible by means of thereductions using normal magnesium having so far been described (L. D.Quinn et al., Tetr. Lett. 26, 2187 (1965). ##STR3##

The high reactivity of the active magnesium having become accessible bythe process according to the present invention is also demonstrated bythe fact that it absorbs hydrogen at a temperature in excess of 150° C.at atmospheric pressure slowly (under a pressure of 2 to 3 bar rapidly)to form magnesium hydride without any need of adding an activator suchas, e.g., in the No. EP-A-0 003 564. These conditions are the mildestconditions under which magnesium has ever been hydrogenated.Commercially available magnesium requires drastic reaction conditions tobe applied in order to accomplish the hydrogenation.

The present invention is further illustrated by, while not limited to,the following examples. All experiments described in the Examples havebeen carried out under argon as protective gas.

EXAMPLE 1

A glass vessel containing 32.0 g of magnesium hydride prepared accordingto the No. EP-A-0 003 564 using a chromium catalyst (Mg:anthracene:CrCl₃=100:1:1; 60° C./20 bar) was heated in an electrically heatableautoclave at from 0.2 to 10 mbar to reach a temperature of 350° C.within 2 hours and then maintained at said temperature until thehydrogen evolution had ceased. The organic components as contained inthe reaction mixture were volatilized in excess of 100° C., while theendothermic hydrogen evolution started at a temperature in excess of250° C. Upon cooling, 28.6 g of a gray pyrophoric magnesium powder wereobtained which had the following composition: Mg 94.5, C 1.4, H 1.3, Cl2.2, Cr 0.5%.

Grignard compounds made from active magnesium: To the suspension of 3.05g (117 mmol) of the thus obtained magnesium powder in 50 ml THF therewere dropwise added 100 mmol of the aryl chloride or allyl chloride RClas set forth in the following Table at the temperature indicated in theTable. After another 30 minutes (during which the temperature was keptconstant in the case of the aryl chlorides and was slowly raised to -10°C. in the case of the allyl chlorides) there was reacted with therespective electrophile and worked up in the conventional manner. Theproducts were identified by comparison of their melting points orboiling points, respectively, IR spectra and ¹ H-NMR spectra with datareported in the literature. ##STR4##

EXAMPLE 2

Reaction of the active magnesium with tetrahyrofuran to form1-oxa-2-magnesia-cyclohexane: A suspension of 2.43 g (95 mmol) of theactive magnesium prepared as described in Example 1 in 75 ml THF washeated to reflux for some days. During this period, samples were takenfrom the solution at defined intervals, hydrolyzed and the yield of1-oxa-2-magnesia-cyclohexane was evaluated by means of the obtainedamount of n-butanol (as determined by gas-chromatography (GC)). Amountof n-butanol found (% of theory) after reaction time (hours; inbrackets): 11.4 (51), 19.6 (99) and 25.4% (243).

In two parallel experiments, suspensions of 2.43 g (95 mmol) of theactive magnesium in 75 ml THF were heated to reflux for 8 days, theexcess of metal was removed by filtration, and to the filtrate therewere added dropwise with stirring 50 mmol trimethylsilyl chloride orbenzoylchloride, respectively, at -78° C.

In the case of the silylation, the reaction mixture was then heated toreflux for 16 hours and thereafter the THF was evaporated under vacuum(14 mbar); the residue was extracted with pentane, the extract wasconcentrated under vacuum (14 mbar), and the remaining liquid wasdistilled at 83° C. to 85° C./14 mbar. There were obtained 3.92 g of4-trimethylsilyl-butoxytrimethylsilane (Speier, J. Am. Chem. Soc. 74,1003 (1952)) (18% based on Mg), which was identified by its ¹H-NMR-spectrum (400 MHz, in CDCl₃): δ (ppm)=-0.05 (s, 9H), 0.08 (s, 9H),0.47 (m, 2H), 1.32 (m, 2H), 1.52 (m, 2H) u. 3.55 (t, 2H).

In the case of the benzoylation, the reaction mixture was heated toreflux for 30 minutes; to the residue obtained after evaporation under14 mbar at room temperature there was added ice water, and the mixturewas extracted with ether. The ether extract was evaporated under vacuumat room temperature, and the remaining oil was distilled at 80° to 85°C./10⁻⁵ bar. There were obtained 3.95 g of 4-benzoylbutylbenzoate(Tsuzumi et al. Jap. Pat. 77, 102, 204; Chem. Abstr. 88, 50515 (1978))(14% based on Mg.), which was identified by its IR and ¹ H-NMR spectra:IR spectrum (film): 1733 and 1695 cm⁻¹. (γC=O); ¹ H-NMR-Spectrum (80MHz, in CDCl₃): δ (ppm)=1.88 (m, 4H), 3.02 (m, 2H), 4.33 (m, 2H),7.2-7.7 (m, 6H) u. 7.75-8.2 (m, 4H).

EXAMPLE 3

2.43 g (0.10 mol) of the commercially available magnesium powder havinga maximum particle diameter of 0.3 mm (50 mesh) were suspended in 0.6 lof absolute THF, and 32.2 g (0.18 mol) of anthracene and 0.06 ml ofethyl bromide were added to the suspension. After 1 hour of stirring atroom temperature the orange precipitate of magnesium anthracene began todeposit. Stirring of the suspension was continued for another 48 hours;after filtration the filtercake was washed three times with 50 ml of THFeach and dried under high vacuum. There were obtained 36.2 g ofmagnesium anthracene.3 THF (86.5%) as an orange microcrystalline powder.

A sample of 10.20 g (24 mmol) of magnesium anthracene.3 THF was firstheated under high vacuum at 100° C. for 1 hour, in the course of whichmainly THF was split off and condensed in a receiver cooled with liquidnitrogen. Then the temperature was increased to 150° C. during 4 hours,in the course of which the removal and sublimation of the anthraceneoccurred. Upon completion of the thermolysis, there were found 4.40 g(83%) of THF (GC analysis) in the receiver cooled with liquid nitrogenand recovered as sublimate 3.57 g (82%) of anthracene which wasidentified by its m.p. of 216° C. and by GC analysis. As the residue ofthe thermolysis there remained 0.52 g (88%) of a highly reactive blackpyrophoric magnesium powder having the following composition (accordingto elementary analysis): Mg 93.6, C 5.3 and H 0.9%.

The specific surface area of the magnesium powder (determined accordingto the BET method, N₂ as the adsorption gas) was 62.3 m² /g.

0,42 g of the thus obtained active magnesium in a H₂ atmosphere undernormal pressure at a temperature of 240° C. absorbed 318 ml of H₂ in thecourse of 2 hours and 358 ml of H₂ after a total of 19 hours (measuredunder 1 bar at 20° C.) to form magnesium hydride (MgH₂). The hydrogenuptake, based on the magnesium content of the sample, was 92%.

EXAMPLE 4

The experiment was carried out as in Example 2, however using the activemagnesium obtained by the thermolysis of magnesium anthracene.3 THF(Example 3). The raction of the active magnesium with THF to form1-oxa-2-magnesia-cyclohexane proceeded at a similar rate as in Example2.

EXAMPLE 5

2.30 g of isobutyl chloride (24.8 mmol) in 30 ml of toluene weredropwise added with stirring to a suspension of 0.65 g (27 mmol) of theactive magnesium prepared according to Example 3 in 100 ml of toluene atroom temperature within 45 minutes, and then the reaction mixture washeated at 70° C. with stirring for 2 hours. The suspension was filtered,and the filtercake was washed with pentane and dried under vacuum (0.2mbar), whereafter 1.69 g of a solid were obtained which had thefollowing composition (according to elementary analysis): C 32.2, H 5.4,Mg 26.4 and Cl 35.9%. 0.3883 g of this solid upon protolysis with2-ethyl-1-hexanol and subsequently with 5N H₂ SO₄ yielded 50.4 ml of agas (0° C./1 bar) having the composition (analysis by mass spectrometry(MS)): isobutane 69.6 and H₂ 30.4%. From the isobutane content of thegas, a yield of isobutylmagnesiumchlorid, based on reacted (see below)isobutyl chloride of 32.7% is calculated. In the toluene solution therewere analyzed (by GC or combined GC and MS analysis, respectively) 0.44g (4.8 mol) of isobutyl chloride, 0.05 g (0.4 mmol) of C₈ H.sub. 18 - (2isomers) and a total of 0.21 g (1.4 mmol) of C₁₁ H₁₆ -hydrocarbons (6isomers, products of the Friedel-Crafts reaction).

In a control experiment, commercially available magnesium powder havinga maximum particle diameter of 0.3 mm (50 mesh) did not display anyreaction with isobutyl chloride under the same conditions (toluene; 70°C.; 2 hours).

EXAMPLE 6

Using 0.71 g (29.2 mmol) of active magnesium (Example 3) and 3.18 g(34.3 mmol) of isobutyl chloride in 130 ml of heptane, however otherwisein analogy of Example 5, the experiment was carried out and the mixtureworked up. After filtration 1.71 g of a solid having the composition C35.2, H 5.8, Mg 23.8 and Cl 35.0% was obtained. Hydrolysis of 0.3908 gof said solid yielded 30.0 ml of isobutane and 14.0 ml of H₂ (20° C./1bar). The yield of isobutylmagnesium chloride, based on reacted (seebelow) isobutyl chloride was 31.6%. In the heptane solution there werefound 1.50 g (16.2 mmol) of isobutyl chloride, 0.06 g (0.5 mmol) of C₈H₁₈ -hydrocarbons (2 isomers) and 0.7 mmol of diisobutylmagnesium(8.3%).

EXAMPLE 7

A distillation apparatus equipped with a dropping funnel was chargedwith 10.4 g (25 mmol) of the magnesium anthracene.3 THF prepared asdescribed in Example 3 in 300 ml of toluene; after stirring for 0.5hours at room temperature the originally orange suspension changed itscolor to green yellow. The suspension was slowly heated to the boilingpoint of the mixture, while, beginning at about 70° C., theprecipitation of a metallic-gray magnesium powder was observed. During 2hours 538 ml of toluene distilled off while, to the same extent as thesolvent distilled, fresh solvent was added dropwise. The precipitatedmagnesium powder was filtered off, washed with toluene and pentane anddried under vacuum (0.2 mbar). There were obtained 0.85 g (71% oftheory) of an active magnesium powder which still contained anthracene.By GC analysis there were determined 5.23 g of THF (97.4% of theory) inthe toluene removed by distillation, and 4.25 g of anthracene (96% oftheory) in the filtrate.

EXAMPLE 8

A distillation apparatus equipped with a gas-introducing tube wascharged with 14.7 g (66 mmol) of magnesium butadiene.2 THF (preparedaccording to Fujita et al. J. Organometal. Chem. 113, 201 (1976)) in 300ml of toluene. In the course of warming up the suspension to the boilingtemperature while passing argon therethrough, the precipitation of themetallic-gray magnesium powder was observed between 50° C. and 80° C.During 90 minutes with the argon stream 173 ml of toluene mixed THF weredistilled; the gaseous products formed during the distillation(butadiene) were collected in a cooled trap (-78° C.) connected to theapparatus. The precipitated magnesium powder was separated byfiltration, washed with toluene and pentane and dried under vacuum (0.2mbar). There were obtained 1.48 g (92% of theory) of an active magnesiumpowder comprising 100% of Mg. 6.2 g of THF and 0.2 g of butadiene werefound in the distilled toluene, and 1.0 g of THF and 1.4 g of butadienewere found in the condensate collected in the trap.

EXAMPLE 9

A solution of 2.2 g (20 mmol) of ethyl bromide in 10 ml of toluene wasdropwise added to a suspension of 8.4 g (20 mmol) magnesium anthracene.3THF in 50 ml of toluene at 0° C. with stirring in the course of 30minutes. The suspension was allowed to warm up to room temperature, andthen the precipitated anthracene was separated by filtration. 20.0 ml(of a total of 60.0 ml) of the solution, under evaporation of thetoluene under vacuum (0.2 mbar) and hydrolysis of the residue withwater, yielded 136 ml (measured under 1 bar at 20° C.) of ethane(according to MS analysis), which correspond to a yield of 85% ofethylmagnesium bromide.

EXAMPLE 10

Using 10.5 g (25 mmol) of magnesium anthracene.3 THF, 1.9 g (25 mmol) ofallyl chloride and 60 ml of THF the experiment was carried out inanalogy of Example 9. The yield of allylmagnesium chloride, determinedby means of the amount of propene formed upon hydrolysis, was 91%.

EXAMPLE 11

Using 4.1 g (9.8 mmol) of magnesium anthracene.3 THF, 0.75 g (9.8 mmol)of allyl chloride and 60 ml of ether the experiment was carried out inanalogy of Example 9. The yield of allylmagnesium chloride, determinedby means of the amount of propene formed upon hydrolysis, was 98%.

EXAMPLE 12

Using 8.4 g (20 mmol) of magnesium anthracene.3 THF, 1.5 g (20 mmol) ofallyl chloride and 60 ml of toluene the experiment was carried out inanalogy of Example 9. The yield of allylmagnesium chloride, determinedby means of the amount of propene formed upon hydrolysis, was 81%.

EXAMPLE 13

A solution of 1.76 g (23 mmol) of allyl chloride in 40 ml of THF wasdropwise added to a suspension of 9.6 g (23 mmol) magnesium anthracene.3THF in 100 ml of THF at -70° C. with stirring in the course of 1 hour,during which period the reaction mixture changed its color into deepblue. The deep blue suspension was subsequently stirred at -70° C. for 8hours. Upon protolysis of the reaction mixture by addition of 5 ml ofmethanol at -70° C., there were recovered 370 ml (measured under 1 barat 20° C.) of propene (according to MS analysis), which correspond to ayield of 67% of allylmagnesium chloride at a reaction temperature of-70° C.

What is claimed is:
 1. A process for preparing a highly reactive finelydivided magnesium comprising thermally decomposing amagnesium-containing compound selected from the group consisting of(i) amagnesium anthracene and/or its derivatives prepared from magnesium andanthracene and/or its alkyl or phenyl derivatives, (ii) a magnesiumbutadiene and/or its alkyl or phenyl derivatives prepared from magnesiumand a conjugated diene having the general formula R¹ -CH=CR² -CH=CH-R³,wherein R¹, R² and R³ are the same or different and represent H, alinear or branched alkyl group having from 1 to 6 carbon atoms or aphenyl residue, and (iii) a magnesium hydride-prepared from magnesiumand hydrogen either in the presence of homogenous catalysts comprising ahalide of a metal of the Subgroups IV to VII of the Periodic System andan organomagnesium compound or a magnesium hydride and in the presenceof a polycyclic aromatic or a tertiary amine, after hydrogenatingmagnesium with magnesium anthracene or magnesium diene, said thermaldecomposition taking place at a pressure from 10⁻⁶ to 1 bar and in theabsence or presence of an organic apretic solvent, either thedecomposition being carried out in the presence of a co-reactant beingadded only after completion of the precipitation of the highly reactivemagnesium, or in the absence of such co-reactant, the magnesium obtainedby said decomposition being isolated as a highly reactive powder.
 2. Theprocess according to claim 1, characterized in that the decomposition ofmagnesium hydride is carried out in the absence of a solvent under apressure of 1 bar at a temperature of from 250° C. to 350° C.
 3. Aprocess according to claim 2, wherein the decomposition is carried outunder a pressure of from 0.2 to 10 mbar and at a temperature of from250° C. to 300° C.
 4. The process according to claim 1, characterized inthat the decomposition of magnesium anthracene.3 THF or an alkyl orphenyl derivative thereof is carried out in the absence of a solventunder a pressure of from 10⁻⁶ to 10³ bar at a temperature of from +70°C. to +170° C.
 5. The process according to claim 1, characterized inthat the decomposition of magnesium anthracene.3 THF or an alkyl orphenyl derivative thereof is carried out in an aliphatic, cycloaliphaticor aromatic hydrocarbon or in an open-chain aliphatic ether, under apressure of 1 bar and at a temperature of from -100° C. to +100° C.
 6. Aprocess according to claim 5, wherein said ether is selected from thegroup consisting of diethylether and dibutylether.
 7. The processaccording to claim 1, characterized in that the decomposition of adductsof magnesium to conjugated dienes of the general formula R¹ -CH=CR²-CH=CH-R³, wherein R¹, R² and R³ are as defined in claim 1, is carriedout in an aliphatic, cycloaliphatic or aromatic hydrocarbon or in anopen-chain aliphatic ether, under a pressure of 1 bar and at atemperature of from -100° C. to +150° C.
 8. A process according to claim7, wherein said ether is selected from the group consisting ofdiethylether and dibutylether.
 9. The process according to claim 1,characterized in that ethyl bromide, 1,2-dichloroethane,1,2-dibromoethane or magnesium halides are used as promoters orcatalysts, respectively, for the decomposition of said thermolabilemagnesium compounds.
 10. Magnesium produced by the process of claim 1.11. The process according to claim 1, characterized in that thedecomposition of adducts of magnesium to conjugated dienes of thegeneral formula R¹ -CH=CR² -CH=CH-R³, wherein R¹, R² and R³ are asdefined in claim 1, is carried out in diethylether or dibutylether undera pressure of 1 bar and at a temperature of from -100° C. to +150° C.